6 A solution of NaOH has a pH of 10.50. How many grams of CaO should be dissolved in sufficient water to make 1.00 L of a solution having the same pH?

Q: 5. How does protonation change the structure of carbonate? (adding a H* to CO;")

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Q: What is the pH of a 7.041 x 10^-6 M HCIO4 solution?

A: Given , concentration of acid solution = 7.041 x 10^-6 M   That means,  [H+] = 7.041 x 10^-6 M

Q: What is the concentration of an aqueous HI solution that has a pH of 2.74?

A: The question is based on the concept of PH calculations.   pH is defined as negative logarithmic of…

Q: 20.0 grams of Sodium hydroxide was dissolved in water up to 500 mL. Calculate the Molar…

A: Given, Grams of sodium hydroxide = 20.0 g Volume of solution = 500 mL       Required,…

Q: 10.T/ An industrial chemist prepares a 0.025 mol/L solution of hydrazoic acid, HN3(aq), a weak…

A:

Q: 2. Describe the variation of the acid strength for the hydrogen halide series and explain which one…

A: Arrange the acids in increasing order of acidic strength--

Q: What is the hydronium ion concentration in an aqueous nitric acid solution with a pH of 3.570?

A:

Q: Question attached

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: What is the pH of a 0.0037 M solution of H2CO3?

A: pH is a negative logarithm of the concentration of H+ ions. A pH scale is used to measure the…

Q: 6. What are the hydrogen and hydroxide 1on concentrations for a solution with a pH value of 4.72?

A: Given data: *pH value of a solution is 4.72.  The relation between concentration of hydrogen ion and…

Q: What is the pH of .03 M NH4Br (aq)? O 3.13 O 9.25 O 10.87 O 1.52 O 5.38

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Q: Calculate the pH of 1M solution of acedic acid (pKa = 4.76)?

A: The pH of the acetic acid solution can be calculated using the formula shown in belowpKa =…

Q: Calculate the pH of a solution containing 0.3 M HCOOH and 0.1 M HCOO (pKa of HCOOH = 3.76)

A: Concentration of HCOOH (Acid) = 0.3 M  Concentration of HCOO- (conjugate base of acid) =  0.1 M  pKa…

Q: What is the pH of 3.7 x 103 M NH¼Br(aq)? Ο 10.4 O 2.4 Ο 11.7 O 5.8 O 4.6

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Q: 8. What are the [H3O+] and [OH–] of Diet Coke that has a pH of 3.17?

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Q: What is the concentration of OH– in a solution with a pH of 3.91?

A: The concentration of OH– in a solution with a pH of 3.91 is to be calculated.

Q: What is the hydronium ion concentration of a solution at 25C with a pOH of 4.7?

A: pH+pOH = 14 pH = -log[H3O+]

Q: which of the following would be a the reaction of Ca o plus NaF

A: When calcium oxide reacts with sodium fluoride gives calcium fluoride and disodium oxide.

Q: What is the pH of a 0.103 M aqueous solution of potassium hypochlorite, KCIO? This solution is pH =

A:

Q: Each day the stomach produces 2.0 L of gastric juice that contains 0.10 M HCl. Phillips Milk of…

A: Given ,  Molarity of HCl (M1) = 0.10 M Volume of HCl (V1) = 0.093 L = 93. mL  Concentration of…

Q: what is the concentration of cl- ions in a 0.1 M solution of calcium chloride?

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Q: A glass of milk has a pH of about 6 and a cup of tea has a pH of 5. Which one has more hydronium…

A: GivenpH of milk = 6pH of tea = 5

Q: What is the hydronium ion concentration in an aqueous perchloric acid solution with a pH of 2.780?…

A: Perchloric acid is a strong mineral acid having chemical formula HClO4.

Q: 2. What is the pH, the pOH and the [OH] of a solution in which the [H*] = 2.43 x 10-6 M? %3!

A: pH is defined as  the negative log of hydrogen ion concentration  pOH is defined as the negative log…

Q: Explain how ammonia can function both as a Brønsted base and as a Lewis base.

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: Which Gas is produced when a metal reacts with dilute hydrochloric acid? Write the chemical reaction…

A: Hydrogen gas is evolved when dilute hydrochloric acid is added to a reactive metal.

Q: Calculate [H,O*] and [OH"'] for the following solutions: pH = 7.41 (Normal blood pH) a. L,OʻH) [OH]…

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Q: Phosphoric acid (H,PO) is a polyprotic acid. Write balanced chemical equations for the sequence of…

A:

Q: 5.) A typical aspirin contains 324 mg of aspirin (HC,H,O4) with Ka = 2.8 x 104. If you dissolve two…

A: pH = -log[H+] Aspirin is a weak acid. For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: 7. A solution of potassium hydrogen sulfite has a pOH = 6.13. The [H1+] is which of the following? *…

A: Potassium hydrogen sulfite  (KHSO3) , on dissociation gives the one H+ ion . pOH = 6.13    We know…

Q: A solution of NaOH has a pH of 10.50. How many grams of CaO should be dissolved in sufficient water…

A: Given data,A) pH of NaOH solution=10.50Volume of Solution=1.0LB) pH of KOH=10.00Volume of…

Q: 1) a) Write the reaction of ammonia with water.

A: ammonia is a colourless gas with a distinct pungent smell.   ammonia (NH3) is a weak base here, H2O…

Q: What is the pH of a 0.130 M solution of HNO₃?b

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Q: Calculate [H3O+] and pH for a 0.317 M solution of HF; Ka = 6.8 × 10−4.

A: Given, Concentration of HF (C) = 0.317 M Dissociation constant of HF , Ka = 6.8×10-4 [H3O+] = ? pH =…

Q: Which of the following statements explain why HBr is a stronger acid than HF? 17

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Q: What is the pH of a 0.35 M solution of hydrofluoric acid with a K, of 6.6 x 104? 3.23 O 1.82 O 5.47…

A: Given: Concentration of HF acid = 0.35 M Ka of HF = 6.6×10-4

Q: Calculate the pH and percent ionization of a 2.5 x 102 45 x 10:4)

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Q: * A solution of NaOH has a pH of 10.50. How many grams of CaO should be dissolved in sufficient…

A:

Q: 6. What is the pH of [OH¯] = 1.0 * 10-5 solution? O 9 1 O 14 O 5

A: Ph Based question first find pOH then find pH

Q: What is the hydronium ion concentration [H3O+] of sea water which has a pH of 8?

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Q: Is Mg(OH)2 a acid, base, or neither?

A: According to the Arrhenius concept of acids and bases :-  Acids donate H+ ions in water and bases…

Q: 3. Write a net ionic equation for the equilibrium that causes the solution of KHTar in water to be…

A: The potassium acid tartrate, KHTar salt is obtained from neutralization reaction of tartaric acid by…

Q: Among the acids of halogens, which is considered to be the most acidic? O HBr Он O H. НЕ О на HCI

A: Given :-  halogen acids : HCl, HBr, HF, HI  To identify :-  most acidic out of the given four acids.

Q: Ag+ (aq)  +  Cl–   (aq)     →     AgCl (s)               Delta H = ? What is the enthalpy change…

A:

Q: Phosphoric acid (H,PO) is a polyprotic acid. Write balanced chemical equations for the sequence of…

A: Phosphoric acid is H3PO4 . It is a polyprotic acid because it has 3 ionizable/replaceable protons.

Q: How many moles of hydroxide ions can be released into solution from 1.00 mg of Mg(OH)2 that is used…

A: Molar mass of Mg(OH)2 = 58.32 g/mol Given mass = 1 mg = 0.001g Moles = 0.001/58.32 = 1.71*10-5

Q: Rank the following in order of increasing acid strength: HIO₃, HI, CH₃COOH, HF.

A: Given, HIO₃, HI, CH₃COOH, HF.

Q: A solution of 1.5 M chlorous acid has a pH of 0.91.  What is the percent ionization of the chlorous…

A: Given, A solution of 1.5 M chlorous acid has a pH of 0.91.  KA = 1.1 x 10−2.

Q: How many mols of HBr are used to neutralize 18.66 mL of a 0.2299 M Ca(OH)₂ solution?

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Q: What is the pH of a 9.5 x 10-4 M HCIO, solution?

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.